Equilibrium Constant Calculation and Naturally Occurring Potassium Isotopes

Equilibrium Constant Calculation

The equilibrium constant, K, for the reaction BaCl₂ (aq) + K₂SO₄ (aq) → BaSO₄ (s) + 2KCl (aq) can be calculated using the formula:

K = [BaSO₄]*[2KCl]/[BaCl₂]*[K₂SO_4}]

Plugging in the given mole values, we get:

K = [3.71 mol/L * (2*4.65 mol/L)] / (2.78 mol/L * 3.25 mol/L) = 8.24

Therefore, the equilibrium constant, K, for the reaction is 8.24 with 3 significant figures.

Naturally Occurring Potassium Isotopes

On Earth, naturally occurring potassium contains the isotopes 39K, 20K, and 41K. The following statements are true for a sample of naturally occurring potassium:

• A mole of naturally occurring potassium has a mass of 39.098 grams
• K-41 has 41 electrons
• All potassium isotopes have more neutrons than protons
• All potassium isotopes have an atomic number of 19
• K−39 is the most abundant potassium isotope
• A mole of K-39 atoms has a mass of 39.098 grams
• Potassium 41 has 19 protons and 22 neutrons

These characteristics define the composition and properties of naturally occurring potassium isotopes.